good oxidizing agent

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Question:Based on what you know about electronegativity which would be a good oxidizing agent?
H2
Cl2
C
Cs

Answers:An oxidizing agent causes other things to oxidize or lose electrons. Cl has the greatest electronegativity for electrons and would cause other elements to give them up.

Question:What makes them "good" oxidizing agents, and whats an example?

Answers:Atoms, ions, and molecules that have an unusually large affinity for electrons tend to be good oxidizing agents.
chemed.chem.purdue.edu/genchem//topicreview/bp/ch19/oxred_3.php - 25k

Question:Using what you know about the electronegativity of the main group elements, which of these would be a good oxidizing agent?
A. H2
B. Cl2
C. C
D. Cs
Please Help!

Answers:B. Cl2
Remember that an oxidizing agent is reduced, it GAINS electrons. Naturally, an element with a HIGH electronegativity, a high tendency for an atom to attract a bonding pair of electrons, would GAIN electrons. Looking at the periodic table, Cl is right next to F, the most electronegative element! Cl has a high electronegativity.
Cesium, on the other hand is the most electropositive element, so it would be a reducing agent. Cesium is really v cool. :)

Question:

Answers:Standard reduction potential [1]:
MnO4 + 8 H+ + 5 e Mn2+ + 4 H2O E = +1.51 V
As you can see it is low in the table
RTlnKeq = nFE so a +ve E means the equilbrium is favored thermodynamically.
If [MnO4]^- is reduced (gain of e-) it must be a strong oxidizing agent (removes e-s).
Another way of looking at it: Mn in [MnO4]^- is formally Mn(VII) its maximum oxdn
state with no d e-. Its preferred oxidation state in H2O is either Mn(II) d^5 or Mn(III) d^4.
But that is thermodynamics and doesn't tell you about the rate of the redox rxn (kinetics).
It is found that redox rxns are usually very fast (an e- is pretty small and doesn't let the
odd atom get in the way of transfer.) Another factor that I haven't seen is that [MnO4]^-
has tetrahedral coordination that probably allows direct contact of the metal center with
the species being oxidized. Mn(II) in H2O is [Mn(H2O)6]^2+ that suggests [(Sub)MnO4]^-
can readily form (Sub is substrate).

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